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| factors that influence reaction rate |
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Definition
| concentration, physical state, temperature |
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| reaction rate in terms of products |
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rate=k[A]^m[b]^n
*m and n are the stoichimetric coefficients if the reaction is elementary... otherwise you have to find them experimentally |
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| how the rate is affected by reactant concentration. |
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| are specific for a particular reaction AT A PARTICULAR TEMPERATURE!!! |
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| units for rate constant k for an overall zeroth order reaction |
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Definition
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| units for a rate constant k for an overall 1st order reaction |
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Definition
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| units for rate constatnt k for an overall second order reaction |
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Definition
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| use of integrated rate laws |
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Definition
| used to solve for concentrations, times, or rate constants when you want to consider time a factor |
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| integrated rate law in straight line form for zeroeth order reaction |
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Definition
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| Integrated rate law in straight line form for a 1st order reaction |
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Definition
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| Integrated rate law in straight line form for a 2nd order reaction |
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Definition
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| half life for a zeroeth order reaction |
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Definition
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| half life for a 1st order reaction |
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Definition
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| half life for a 2nd order reaction |
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Definition
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Definition
k=Ae^(-Ea/RT)
A=frequency factor |
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| What happens as T increases, according to the Arrhenius equation? |
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Definition
| k increases, and therefore the rate increases. |
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| If the Ea forward is larger than the Ea reverse, is the process endothermic or exothermic? |
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Definition
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| If the Ea reverse is larger than the Ea forward, is the reaction endothermic or exothermic? |
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| According to the Arrhenius equation, as Ea increases, what happens to k and rate? |
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Definition
| k decreases, which leads to a decreased rate. |
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| what is a spontaneous reaction? |
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Definition
| one proceeding towards equilibrium. |
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what is the sign of ΔS for the following rxns:
solid-->liquid--> gas
crystalline solid + liquid-> ions
crystaline solids-> gases + ions |
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Definition
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Definition
| each quantized state of a system (energy levels) |
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| equations for ΔS of a system |
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Definition
ΔS (sys)=q/T
** RECAll q= cmΔT!!!!!! |
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| Entropy in similar compounds |
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Definition
| for similar compounds, entropy increases with molar mass |
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| determining spontaneity using entropy |
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Definition
ΔS (universe)>0 means spontaneous
** note... must take into consideration ENTIRE univers, so ΔS sys+ ΔS surr |
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| entropy in relationship to equilibrium |
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Definition
ΔS (univ)=0 therefore
ΔS (sys)=-ΔS (surr) |
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| phase changes in relationship to equilibrium |
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Definition
| phase changes occur at equilibrium |
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Definition
ΔG=ΔH-TΔS
**WOrd of Caution-- if rxn is not at 298 k, then you MUST use this formula, because the tables are made at 298 K!!!! |
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| spontaneity in relation with gibbs free energy |
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Definition
ΔG<0 spontaneous
ΔG>0 nonspontaneous
ΔG=0 equilibrium |
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Definition
| the heat required to heat one gram of water by 1 C. |
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| does vapor pressure for a liquid increase as the temperature increases? |
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Definition
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| do fast reactions have large equilibrium constants? |
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Definition
| not necessarily. Keq=K1/K(-1), and the reaction could occur quickly in both directions. |
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| are activation energies for forward and reverse reactions the same? |
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Definition
| nope. draw some pictures. |
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| will the equilibrium constant for a reaction increase if a catalyst is added? |
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Definition
| nope, catalysts only affect the activation energy. |
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| are the rates of forward and reverse reactions equal at equilibrium? |
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Definition
| yes, this is the definition of equilibrium |
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Definition
| when the reaction rates for the forward and reverse processes are equal |
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| 1st law of thermodynamics |
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| adding oxygen gas to form carbon dioxide and water |
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| ΔH(soln)=ΔH(solute) + ΔH(solvent) + ΔH(mix) |
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Definition
| ΔH(soln)=ΔH(lattice)+ΔH(hydration) |
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Definition
pi=MRT
M=molarity
R=gas constant
pi=osmotic pressure |
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| charge density: periodic trends |
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Definition
charge density increases as you move across the periodic table, and decreases as you move down
inc
-------->
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| dec
\/ |
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Definition
| solute and solvent are soluble in each other in any proportion. |
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| list these major types of intermolecular forces in order of decreasing strength: dipole-dipole, H bond,ion-induced dipole, dipole induced dipole,ion-dipole, dispersion |
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Definition
| ion-dipole, H bond, Dipole-dipole, ion-induced dipole, dipole-induced diole, dispersion. |
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| what kind of intermolecular forces are seen with the use of soap to remove grease? |
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Definition
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| how is charge density related to heat of hydration? |
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Definition
| the higher the charge density,the more negative ΔH (hydration) is |
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Definition
| a thermodynamic variable directly related to the number of ways that a system can distribute its energy. |
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| gas solubility and rising temperature |
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Definition
| gas solubility in water decreases with rising temperature |
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